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- Was the gradual color change observed when the sodium thiosulfate (Na2S2O3) crystal was added to the aqueous solution of KI/12 in Station Cevidence of a chemical or physical change?Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32Balance the following chemical equation using the smallest possible wholenumber coefficients: P4 + Cl2 → PCl3A. 2 P4 + 6 Cl2 → 8 PCl3B. P4 + Cl2 → 4 PCl3C. P4 + 6 Cl2 → 4 PCl3D. P4 + 16 Cl2 → 4 PCl3
- In the synthesis of benzoic acid, 3.5 mL of toluene were used and mixed with potassium permanganate solution. In making the potassium permanganate solution, 7 grams of the powder were dissolved in 150 mL of water. The resulting crystals were purified and the yield 1.53 grams. Identify the limiting reagent and compute for the number of moles that it consumed. What is the theoretical yield? What is the percentage yield? MW toluene = 94.14, density=0.87 g/mL , MW KMnO4 = 158, density = 2.7 g/mL , MW Benzoic acid = 122, density = 1.27 g/mLVanadic ion, V3+, forms green salts and is a good reducingagent, being itself changed in neutral solutions to thenearly colorless ion V(OH)4+. Suppose that 15.0 mL of a0.200-M solution of vanadic sulfate, V2(SO4)3, was neededto reduce completely a 0.540-g sample of an unknownsubstance X. If each molecule of X accepted just oneelectron, what is the molecular weight of X? Suppose thateach molecule of X accepted three electrons; what wouldbe the molecular weight of X then?A technician is setting up a laboratory to standardise ~0.0200 mol dm–3 KMnO4. What mass of Mohr’s salt [FeSO4(NH4)2SO4·6H2O] would the technician be required to weigh out to produce a 5.00 L solution of Mohr’s salt such that 25.0 cm3 aliquots of the salt would require a titre of 20.0 cm3 to standardise the KMnO4 solution?
- 1. Write a balanced equation for the reaction between sodium carbonate (Na2CO3) andhydrochloric acid (HCl).2. Calculate the theoretical yield (in grams) of the CO2 that should be produced from the massof Na2CO3 used. Use dimensional analysis.3. Use the following equation to calculate the percent yield of the CO2.experimental(actual) %yield x 100theoretical(calculated)=4. Calculate the theoretical yield of NaCl from the amount of Na2CO3 used. Use dimensionalanalysis.5. Use the following equation to calculate the percent yield of the NaCl in your experiment.experimental(actual) %yield x 100theoretical(calculated)What constitutes a 'reference material', and why does its utilization play a criticalrole in the chemical analysis of food products? Provide examples.Which are characteristics of a primary standard? has an anhydrous form as a well as hydrated form low cost stability in the atmosphere high purity low molar mass high molar mass low solubility
- The mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)Souring of wine occurs when ethanol is converted to acetic acid by oxygen: C2H5OH(l) +O2(g)--->CH3COOH(g)+H2O(l). A 1.00 L bottle of wine labeled as 7.00% (%v/v) ethanol, is found to have a defective seal. Analysis of 1.00 mL showed that there were 0.0274 g acetic acid in that 1.00 mL. The density of ethanol is 0.816 g/mL. (a) What mass of oxygen must leaked into the bottle in pounds(lb) (b) What is the percent yield for the conversion of ethanol to acetic acid, if oxygen is in excess2.Acrude compound with a mass of 0.62667 g was recrystalised to give 0.1352 g of crystals . Calculate the percentage recovery .Suggest possible reasons for the low percentage recovery